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General Chapter 5 Review
This is a general review for the material covered in this chapter. It is intended to be
a supplementary study tool that should be used in conjunction with all notes,
worksheets, and your text. Please show all work and circle your final answer for full
credit. (88 PTS.)
1. Define the following:
a. Kinetic energy:
b. Formula for kinetic energy (identify the variables and their units):
c. 1 calorie = ___________ Joule
d. Potential energy
e. State Function
f. Specific heat
g. Heat capacity
h. Calorimeter
2. Draw a picture of an exothermic system having work done on it by the surroundings.
Label system, surroundings, heat, and work.
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3. What is the first law of thermodynamics?
4. A system releases 437.00 kJ of heat and 467.00 J of work are done on the system.
What is the internal energy of the process? Is this process exothermic or endothermic?
5. Circle the following that ARE state functions
Heat
Work
Internal energy
Potential energy
Kinetic energy
Enthalpy
Time
Temperature
6. What form of work is present in the thermodynamic function of enthalpy?
7. Draw an enthalpy diagram for an exothermic reaction, include the ΔH value.
8. Draw an enthalpy diagram for an endothermic reaction, include the ΔH value.
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9. How much heat is released when 6.50 g of oxygen gas is burned in a constant
pressure system according to the equation below? BECAREFUL!
CH4 (g) + O2 (g)  CO2 (g) + H2O (l)
ΔH = -890 kJ
10. How much heat is needed to warm 250.0 g of water from 22.0 °C to 98.0 °C.
11. The specific heat of calcium is 0.179 J/g-K. How many J of heat are necessary to
raise the temperature of 1.42 kg block of calcium from 35.0 °C to 98.0 °C?
12. The specific heat of benzene is 2.34 J/g-K. How many Joules of heat are needed
to raise the temperature of 63.0 g of benzene from 16.0 °C to 38.0 °C?
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13. When 4.04 g of solid ammonium nitrate dissolve in 60.0g of water in a coffee cup
calorimeter. The temperature of the water drops from 23.0°C to 16.0 °C.
Calculate change in enthalpy for the solution in kJ/mol of NH4NO3.
NH4NO3 (g)  NH4+ (aq) + NO3- (aq)
15.
Use the thermochemical equations shown below to determine
the enthalpy for the reaction:
N2(g) + 3H2(g) 2NH3(g)
H= - 184.0 kJ
N2(g) + 2O2(g)  2NO2(g)
H= - 132.0 kJ
H2(g) + 1/2O2(g)  H2O(l)
H= 70.0 kJ
2NO2(g) + 7H2(g)  2NH3(g) + 4H2O(l) H=
16. Use the thermochemical equations shown below to determine
the enthalpy for the reaction:
H2CO3  H2CO + O2
H= 140.0 kJ
H2O + CO2  H2CO + O2
H= 62.5 kJ
H2O + CO2  H2CO3
H=
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Use table appendix 3 to answer the following questions.
17. Identify the standard state (solid, liquid or gas) for the following elements:
Place an X in the box if a value is not given.
UNITS_______________________
***Solid***
Liquid- aq
Gas
Carbon
dioxide
sodium
water
KOH
Sulfuric
Acid
18. Calculate the ΔH° for the reaction:
2CH3OH (l) + 3O2 (g)  2CO2 (g) + 4H2O (l)
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